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Problem- A reaction is second order in X and zero order in Y. Doubling the initial concentration of X and having the initial concentration of Y at constant temperature causes the initial rate to:
(1) increase by a factor of 4.
(2) decrease by a factor of 2.
(3) remain unchanged.
(4) increase by a factor of 2.
(5) be undeterminable without the balanced equation.
I need help for above question. Show each steps for the above problem.
The heat of combustion of CH4 is 8904 kJ/mol also the heat capacity of H2O is 75.2 J/mol×K. Determine the volume of methane measured at 298 K and 0.790atm needed to convert 1.33L of water at 298 K to water vapor at 373 K.
The next 6 questions involve the calculation of concentrations of the molecular and ionic species in an aqueous solution that has an analytical composition of 0.260 M KH2PO4 + 0.160 M K2HPO4.
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A certain reaction has activation energy of 39.37 kJ/mol. Explain at what Kelvin temperature will the reaction proceed 4.00 times faster than it did at 337 K. Explain out how you did it
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When a strong acid and strong base titration is not at equivalence, the pH can be found by finding the number of moles of H3O+ or OH- in excess, converting to [H3O+] or [OH-], and solving for the pH.
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