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#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 :)
 one year ago
 one year 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 :)
 one year ago
 one year ago

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iheartfoodBest 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 :/
 one year ago

iheartfoodBest ResponseYou've already chosen the best response.0
is it 4?? or is it 3? ;/
 one year ago

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

iheartfoodBest 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 =/
 one year ago

iheartfoodBest 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 :/
 one year ago

UnkleRhaukusBest ResponseYou've already chosen the best response.1
one at a time please
 one year ago

iheartfoodBest 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?
 one year ago

iheartfoodBest ResponseYou've already chosen the best response.0
oh 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?
 one year ago

iheartfoodBest ResponseYou've already chosen the best response.0
so what do i do now? and is this #1 right?
 one year ago

UnkleRhaukusBest 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 \(\text{KMnO}_4\) \[M_{\text{KMnO}_4}=M_{\text K}+M_{\text{Mn}}+4M_{\text O}=\]
 one year ago

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

iheartfoodBest ResponseYou've already chosen the best response.0
okay so what's after that? how do i see what percentage it is?
 one year ago

UnkleRhaukusBest ResponseYou've already chosen the best response.1
have you worked out the molar mass of KMnO4?
 one year ago

iheartfoodBest ResponseYou've already chosen the best response.0
noo ;( idk how to do that :(
 one year ago

UnkleRhaukusBest ResponseYou've already chosen the best response.1
\[M_{\text{KMnO}_4}=M_{\text K}+M_{\text{Mn}}+4M_{\text O}=\]
 one year ago

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

UnkleRhaukusBest ResponseYou've already chosen the best response.1
maybe it is best to try these when you aren't so tired
 one year ago

iheartfoodBest ResponseYou've already chosen the best response.0
oaky :) i will!! thank youuu :D
 one year ago
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