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CHEM1011-Chemistry 1A (T3 2026)
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At elevated temperatures, molecular hydrogen and molecular bromine react to partially form hydrogen bromide:
H2 (g) + Br2 (g) ⇌ 2HBr (g)A mixture of 0.48 mol of H2 and 0.725 mol of Br2 is combined in a reaction vessel with a volume of 2.00 L. At equilibrium, there are 0.299 mol of H2 present. At equilibrium, there are ________ mol of Br2 present in the reaction vessel.
Consider the following equilibrium reaction:
H2CO3 (aq) ⇌ H+ (aq) + HCO3– (aq); K = 5.0 x 10–7
If the initial concentrations of the species are:
[H2CO3] = 0.12 M; [H+] = 5.00 x 10–5 M; [HCO3–] = 4.00 x 10–3 M
Which one of the statements below describes the relationship between Q and K and then the correct direction of chemical change?
Consider the reaction below, for which K = 794 at 25 °C.
H2 (g) + I2 (g) ⇌ 2 HI (g) What is the value of K for the equilibrium below?½ H2 (g) + ½ I2 (g) ⇌ HI (g)
In which of the following reactions would increasing pressure at constant temperature NOT change the concentrations of reactants and products, based on Le Châtelier's principle?
Nitrosyl bromide decomposes according to the following equation:
2NOBr (g) ⇌ 2NO (g) + Br2 (g)
A sample of NOBr (0.614 mol) was placed in an empty 1.00 L flask. At equilibrium the flask contained 0.159 mol of NOBr. How many moles of NO are in the flask at equilibrium?
Given the following reaction:
CO (g) + 2H2(g) ⇌ CH3OH (g)
In an experiment, 0.42 mol of CO and 0.42 mol of H2 were placed in a 1.00 L reaction vessel. At equilibrium, there were 0.29 mol of CO remaining. KC for the reaction is ________.
Consider the following equilibrium reaction:
H2CO3 (aq) ⇌ H+ (aq) + HCO3– (aq); K = 5.0 x 10–7
If the initial concentrations of the species are:
[H2CO3] = 0.010 M; [H+] = 1.2 x 10–5 M; [HCO3–] = 4.0 x 10–3 M
Which one of the statements below describes the relationship between Q and K and then the correct direction of chemical change?
Consider the reaction below, for which K = 0.212 at 100°C.
N2O4 (g) ⇌ 2 NO2 (g)
What is the value of K at this temperature for the following reaction?
2 NO2 (g) ⇌ N2O4
Consider the following exothermic reaction at equilibrium:
2SO2 (g) + O2 (g) ⇌ 2SO3 (g) ΔH° = –99 kJ/mol
Le Châtelier's principle predicts that an increase in temperature at constant pressure will result in ________.
Nitrosyl bromide decomposes according to the following equation:
2NOBr (g) ⇌ 2NO (g) + Br2 (g)
A sample of NOBr (0.715 mol) was placed in an empty 1.00 L flask. At equilibrium the flask contained 0.182 mol of NOBr. How many moles of Br2 are in the flask at equilibrium?