anonymous
  • anonymous
#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 :)
Chemistry
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schrodinger
  • schrodinger
I got my questions answered at brainly.com in under 10 minutes. Go to brainly.com now for free help!
anonymous
  • anonymous
#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
  • anonymous
idk :(
anonymous
  • anonymous
is it 4?? or is it 3? ;/

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anonymous
  • anonymous
idk how to do that :/ can u pls show me? and this if for #1 right>?
anonymous
  • anonymous
#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
  • anonymous
#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
  • UnkleRhaukus
one at a time please
anonymous
  • anonymous
#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
  • anonymous
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?
UnkleRhaukus
  • UnkleRhaukus
ok,
anonymous
  • anonymous
so what do i do now? and is this #1 right?
UnkleRhaukus
  • UnkleRhaukus
#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
  • UnkleRhaukus
\[M_{\text K}=39 \quad\text g /\text{mol}\]\[M_{\text {Mn}}=55 \quad\text g /\text{mol}\]\[M_{\text {O}}=16 \quad\text g /\text{mol}\]
anonymous
  • anonymous
okay so what's after that? how do i see what percentage it is?
UnkleRhaukus
  • UnkleRhaukus
have you worked out the molar mass of KMnO4?
anonymous
  • anonymous
noo ;( idk how to do that :(
UnkleRhaukus
  • UnkleRhaukus
\[M_{\text{KMnO}_4}=M_{\text K}+M_{\text{Mn}}+4M_{\text O}=\]
anonymous
  • anonymous
ohh but idk what to do there :/ at least not on this one :(
UnkleRhaukus
  • UnkleRhaukus
maybe it is best to try these when you aren't so tired
anonymous
  • anonymous
oaky :) i will!! thank youuu :D

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