1. HI -----> 1/2 H2+ 1/2 I2 In zero order in HI with a rate constant of 1.20 x 1
ID: 926427 • Letter: 1
Question
1. HI -----> 1/2 H2+ 1/2 I2 In zero order in HI with a rate constant of 1.20 x 10^-4 Ms^-1 If the initial concentration of HI is 0.110 M, the concentration of HI will be 2.43 x 10^-2 M after _____seconds have passed. 2. Put in order from lowest to highest boiling point. 0.17 m Ba(NO3)2, 0.14 m Fe(CH3COO2), 0.15 m CrCl2, 0.49 m Sucrose( nonelectrolyte) 3. The hydroxide ion concentration of an aqueous solution of 0.558 M formic acid, HCOOH is.... OH- = ________ M 5. The hydroxide ion concentration[OH-], of an aqueous solution of 0.524 M dimethylamine( a weak base with the formula (CH3)2NH), kb= 5.9 x 10^-4, is: OH- = _______ M1. HI -----> 1/2 H2+ 1/2 I2 In zero order in HI with a rate constant of 1.20 x 10^-4 Ms^-1 If the initial concentration of HI is 0.110 M, the concentration of HI will be 2.43 x 10^-2 M after _____seconds have passed. 2. Put in order from lowest to highest boiling point. 0.17 m Ba(NO3)2, 0.14 m Fe(CH3COO2), 0.15 m CrCl2, 0.49 m Sucrose( nonelectrolyte) 3. The hydroxide ion concentration of an aqueous solution of 0.558 M formic acid, HCOOH is.... OH- = ________ M 5. The hydroxide ion concentration[OH-], of an aqueous solution of 0.524 M dimethylamine( a weak base with the formula (CH3)2NH), kb= 5.9 x 10^-4, is: OH- = _______ M
In zero order in HI with a rate constant of 1.20 x 10^-4 Ms^-1 If the initial concentration of HI is 0.110 M, the concentration of HI will be 2.43 x 10^-2 M after _____seconds have passed. 2. Put in order from lowest to highest boiling point. 0.17 m Ba(NO3)2, 0.14 m Fe(CH3COO2), 0.15 m CrCl2, 0.49 m Sucrose( nonelectrolyte) 3. The hydroxide ion concentration of an aqueous solution of 0.558 M formic acid, HCOOH is.... OH- = ________ M 5. The hydroxide ion concentration[OH-], of an aqueous solution of 0.524 M dimethylamine( a weak base with the formula (CH3)2NH), kb= 5.9 x 10^-4, is: OH- = _______ M
Explanation / Answer
There are multiple questions here . i am allowed to answer only 1 at a time. I will answer 1st one for you. Please ask other as different question
1.
For Zero order reaction,
[Ro] - [R] = K*t
0.11 - 2.43*10^-2 = 1.2*10^-4 * t
t= 714.2 s
Answer: 714.2 s
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