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anonymous
 3 years ago
#1: The theoretical yield of a reaction is 5.00 moles of potassium permanganate (KMnO4). If the reaction actually produces 695.2 g KMnO4, what is the percent yield of the reaction?
A. 78%
B. 83%
C. 88%
D. 120%
**idk :( which is it? @UnkleRhaukus :)
anonymous
 3 years ago
#1: The theoretical yield of a reaction is 5.00 moles of potassium permanganate (KMnO4). If the reaction actually produces 695.2 g KMnO4, what is the percent yield of the reaction? A. 78% B. 83% C. 88% D. 120% **idk :( which is it? @UnkleRhaukus :)

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anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0#2: The equation for the formation of water from hydrogen gas and oxygen gas is 2H2 + O2 2H2O. How many grams of water can be made from 160 g of oxygen gas? A. 160 g B. 180 g C. 320 g D,. 405 g **idk this one either :/

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0is it 4?? or is it 3? ;/

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0idk how to do that :/ can u pls show me? and this if for #1 right>?

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0#3: Consider the hydrazinenitrogen tetroxide rocket fuel reaction: 2N2H4 + N2O4 3N2 + 4H2O How many grams of N2H4 will be consumed by 92 g of N2O4? A. 128 g B. 64 g C. 32 g D. 16 g **my answer; C. 32 g is that right?? not too sure =/

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0#4: Consider this reaction: N2 + 3H2 2NH3 Suppose you have 2.0 L of nitrogen. How many liters of hydrogen do you need for a complete reaction? (One mole of any gas occupies 22.4 L under certain conditions of temperature and pressure. Assume those conditions for this question.) A. 2.6 L B. 6.0 L C. 9.0 L D. 10.0 L **my answer: A. 2.6 L is that right?? again, not too sure :/

UnkleRhaukus
 3 years ago
Best ResponseYou've already chosen the best response.1one at a time please

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0#5: A reaction produces 10.5 L of oxygen, but was supposed to produce 1 mol of oxygen. What is the percent yield? (One mole of any gas occupies 22.4 L under certain conditions of temperature and pressure. Assume those conditions for this question.) A. 22% B. 47% C. 67% D. 94% **my answer; B. 47% is that right?

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0oh oaky sorry!! btw, that's all the questions so ill just leave em there and we can scroll up! is that oaky? and oaky i seee... what do i do next?

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0so what do i do now? and is this #1 right?

UnkleRhaukus
 3 years ago
Best ResponseYou've already chosen the best response.1#1: how many moles is \(695.2 [\text g] \text{KMnO}_4\) ? first you need to work out the molar mass of \(\text{KMnO}_4\) \[M_{\text{KMnO}_4}=M_{\text K}+M_{\text{Mn}}+4M_{\text O}=\]

UnkleRhaukus
 3 years ago
Best ResponseYou've already chosen the best response.1\[M_{\text K}=39 \quad\text g /\text{mol}\]\[M_{\text {Mn}}=55 \quad\text g /\text{mol}\]\[M_{\text {O}}=16 \quad\text g /\text{mol}\]

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0okay so what's after that? how do i see what percentage it is?

UnkleRhaukus
 3 years ago
Best ResponseYou've already chosen the best response.1have you worked out the molar mass of KMnO4?

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0noo ;( idk how to do that :(

UnkleRhaukus
 3 years ago
Best ResponseYou've already chosen the best response.1\[M_{\text{KMnO}_4}=M_{\text K}+M_{\text{Mn}}+4M_{\text O}=\]

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0ohh but idk what to do there :/ at least not on this one :(

UnkleRhaukus
 3 years ago
Best ResponseYou've already chosen the best response.1maybe it is best to try these when you aren't so tired

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0oaky :) i will!! thank youuu :D
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