The reaction X + Y --> products was studied using the method of initial rates. The initial rate of consumption of X was measured in three different experiments. What is the value of the rate constant, k? *concentrations are in
Calculate the heat of formation of SiO4(s), given that the heats of formation of SiO2(s), -910.90 KJ/mol; H2O(l), -285.8 KJ/mol; HF (g), -271.1 KJ/mol. I know the heat of formation is products minus reactants but how do i do this
Chemistry HELP - Rates of reaction, redox reactions? 10 points? An structural isomer of bromobutane (C4H9Br) can be hydrolysed using aqueous sodium hydroxide to produce butanol. This can be represented by the following equation:
Rates of reaction, redox reactions? 10 points? An structural isomer of bromobutane (C4H9Br) can be hydrolysed using aqueous sodium hydroxide to produce butanol. This can be represented by the following equation: C4H9Br(l) +
Nitric oxide reacts with bromine gas at elevated temperatures according to the equation, 2 NO(g) + Br2(g) = 2 NOBr(g) The experimental rate law is rate = k[NO][Br2]. In a certain reaction mixture the rate of formation of NOBr(g)
From the reaction below, calculate the free energy of formation for C3H6(g) at 25°C, if ΔGfo(CH4(g)) is -50.790 kJ/mol. 3CH4(g) ↔ C3H6(g) + 3H2(g) ΔGo = 215.302 kJ/mol i've tried doing final-initial, and products
i need help with this pre lab question:| plse help me! teh following data were obained for the reaction 2ClO2(aq)+ 2OH^-(aq) -> ClO3^-(aq) + ClO2^-(aq) +H2O (l) Where rate = delta[ClO2]/ delta t (mol/L) (mol/L) (mol/L*s)
The reaction between NO (nitric oxide) and oxygen is a key step in the formation of acid rain. O2(g) + 2NO(g) → 2NO2(g) A series of experiments were run, each of which starts with a different set of reactant concentrations.