Name……………………………………............................. Index number
... 17. A student prepared ammonia gas and allowed it to pass into a solution of zinc sulphate as shown in the set- up below. ...
... 17. A student prepared ammonia gas and allowed it to pass into a solution of zinc sulphate as shown in the set- up below. ...
4. Sodium nitrite (NaNO2) is a controversial food preservative added
... 10. A gaseous mixture containing 7.50 mol H2(g) and 9.00 mol Cl2(g) reacts to form hydrogen chloride (HCl) gas. a) Write a balanced equation for the reaction. b) Which reactant is limiting? c) If all the limiting reactant is consumed, how many moles of hydrogen chloride are formed? d) How many moles ...
... 10. A gaseous mixture containing 7.50 mol H2(g) and 9.00 mol Cl2(g) reacts to form hydrogen chloride (HCl) gas. a) Write a balanced equation for the reaction. b) Which reactant is limiting? c) If all the limiting reactant is consumed, how many moles of hydrogen chloride are formed? d) How many moles ...
Biol 1020 Ch. 2 Chemistry
... Oxidation-Reduction Reactions Are Common in Biological Systems example: rusting ...
... Oxidation-Reduction Reactions Are Common in Biological Systems example: rusting ...
3 - Rates
... The reaction is spontaneous at 298K It is exothermic entropy is decreasing enthalpy is decreasing the names and states of reactants and products are given for every 3 mol of H2(g) and 1 mol of N2(g) consumed 2 mol of NH3(g) is ...
... The reaction is spontaneous at 298K It is exothermic entropy is decreasing enthalpy is decreasing the names and states of reactants and products are given for every 3 mol of H2(g) and 1 mol of N2(g) consumed 2 mol of NH3(g) is ...
Balancing a Chemical Equation
... Chemical Equations In many chemical reactions, a catalyst is added to the reaction mixture. • A catalyst is a substance that speeds up the reaction but is not used up in the reaction. • A catalyst is neither a reactant nor a product, so its formula is written above the arrow in a chemical equation. ...
... Chemical Equations In many chemical reactions, a catalyst is added to the reaction mixture. • A catalyst is a substance that speeds up the reaction but is not used up in the reaction. • A catalyst is neither a reactant nor a product, so its formula is written above the arrow in a chemical equation. ...
Chemical Equilibrium
... A Note about Units Notice that I wrote the equilibrium constant without units even though the concentrations have units: ...
... A Note about Units Notice that I wrote the equilibrium constant without units even though the concentrations have units: ...
Lecture 1 and 2a - Thermochemistry
... from the initial state and the final state. ΔE, however, is a state function, which means that the value of ΔE depends only on the initial and final states and not the path taken. ΔE can be calculated as Efinal – Einitial. Many chemical reactions and processes are carried out at constant pressure, s ...
... from the initial state and the final state. ΔE, however, is a state function, which means that the value of ΔE depends only on the initial and final states and not the path taken. ΔE can be calculated as Efinal – Einitial. Many chemical reactions and processes are carried out at constant pressure, s ...
calculations of mechanical work in 1, 2 and 3 dimensions
... A chemical reaction with methanol creates heat in the NiTi alloy wire. At a higher temperature, the wire’s length shrinks - thus lifting a weight and doing work on the surroundings. V.H. Ebron et al., Science (2006) 311, 1580 ...
... A chemical reaction with methanol creates heat in the NiTi alloy wire. At a higher temperature, the wire’s length shrinks - thus lifting a weight and doing work on the surroundings. V.H. Ebron et al., Science (2006) 311, 1580 ...
The adiabatic flame temperature
... in the quenching of the chain propagating reactions. As the pressure increases: molecular mean free path decreases and O, H, OH radicals begin to react with other species. At some pressure (~1.5mmHg for 500°C), chain-propagating reactions prevail over wall destruction and the mixture can explode. 2n ...
... in the quenching of the chain propagating reactions. As the pressure increases: molecular mean free path decreases and O, H, OH radicals begin to react with other species. At some pressure (~1.5mmHg for 500°C), chain-propagating reactions prevail over wall destruction and the mixture can explode. 2n ...
7.1 Equilibrium PPT equilibrium1
... pressure is increased? Explain. 2) State and explain three (3) ways the amount of NO2 production can be increased. ...
... pressure is increased? Explain. 2) State and explain three (3) ways the amount of NO2 production can be increased. ...
Review Worksheet
... c) These particles are considered to be dimensionless points which occupy zero volume. The volume of real gas molecules is assumed to be __________ for most purposes. This above statement is NOT TRUE. Real gas molecules do occupy volume and it does have an impact on the behavior of the gas. This imp ...
... c) These particles are considered to be dimensionless points which occupy zero volume. The volume of real gas molecules is assumed to be __________ for most purposes. This above statement is NOT TRUE. Real gas molecules do occupy volume and it does have an impact on the behavior of the gas. This imp ...
EKSIKA JOINT EVALUATION TEST. Kenya Certificate
... Given that the lattice enthalpy of potassium chloride is +690KJ/mol and hydration enthalpies of K+ and Cl- are -322KJ and -364KJ respectively. Calculate the enthalpy of solution of potassium chloride. ...
... Given that the lattice enthalpy of potassium chloride is +690KJ/mol and hydration enthalpies of K+ and Cl- are -322KJ and -364KJ respectively. Calculate the enthalpy of solution of potassium chloride. ...
MS PowerPoint - Catalysis Eprints database
... where, , the switching factor, reads 0 below the threshold and 1 above it. Refinement, the electronic parameter: Property = a(d) + b(θ – θth) + c(Ear) + d(p) + e where d is used for -donicity and p used for -acceptor property; Ear is for “aryl effect”. For reactions having a simple rate equa ...
... where, , the switching factor, reads 0 below the threshold and 1 above it. Refinement, the electronic parameter: Property = a(d) + b(θ – θth) + c(Ear) + d(p) + e where d is used for -donicity and p used for -acceptor property; Ear is for “aryl effect”. For reactions having a simple rate equa ...
Chapter 2 The Chemical Context of Life About 25 of the 92 natural
... D) outer-shell electrons of one atom are transferred to fill the inner electron shell of another atom. E) an electron occupies a hybrid orbital located between the nuclei of two atoms. Answer: C Topic: Concept 2.3 8. Which of the following correctly describes chemical equilibrium? A) Forward and rev ...
... D) outer-shell electrons of one atom are transferred to fill the inner electron shell of another atom. E) an electron occupies a hybrid orbital located between the nuclei of two atoms. Answer: C Topic: Concept 2.3 8. Which of the following correctly describes chemical equilibrium? A) Forward and rev ...
Transition state theory
Transition state theory (TST) explains the reaction rates of elementary chemical reactions. The theory assumes a special type of chemical equilibrium (quasi-equilibrium) between reactants and activated transition state complexes.TST is used primarily to understand qualitatively how chemical reactions take place. TST has been less successful in its original goal of calculating absolute reaction rate constants because the calculation of absolute reaction rates requires precise knowledge of potential energy surfaces, but it has been successful in calculating the standard enthalpy of activation (Δ‡Hɵ), the standard entropy of activation (Δ‡Sɵ), and the standard Gibbs energy of activation (Δ‡Gɵ) for a particular reaction if its rate constant has been experimentally determined. (The ‡ notation refers to the value of interest at the transition state.)This theory was developed simultaneously in 1935 by Henry Eyring, then at Princeton University, and by Meredith Gwynne Evans and Michael Polanyi of the University of Manchester. TST is also referred to as ""activated-complex theory,"" ""absolute-rate theory,"" and ""theory of absolute reaction rates.""Before the development of TST, the Arrhenius rate law was widely used to determine energies for the reaction barrier. The Arrhenius equation derives from empirical observations and ignores any mechanistic considerations, such as whether one or more reactive intermediates are involved in the conversion of a reactant to a product. Therefore, further development was necessary to understand the two parameters associated with this law, the pre-exponential factor (A) and the activation energy (Ea). TST, which led to the Eyring equation, successfully addresses these two issues; however, 46 years elapsed between the publication of the Arrhenius rate law, in 1889, and the Eyring equation derived from TST, in 1935. During that period, many scientists and researchers contributed significantly to the development of the theory.