for Chemistry:
What volume will be occupied by a sample of hydrogen at 1.51 atm if the volume at 740 mmHg is 223 mL (constant temp)?
I was using the formula (P1)(V1)/(n1)(T1) = (P2)(V2)/(n2)(T2)
I concluded (perhaps incorrectly) that the n's and T's cancel out since there is no change at all.
I then calculated (again perhaps incorrectly) that the V2 was equal to 143.84 mL.
Can someone check my answer or tell me how to solve it? Thank you in advance!
What volume will be occupied by a sample of hydrogen at 1.51 atm if the volume at 740 mmHg is 223 mL (constant temp)?
I was using the formula (P1)(V1)/(n1)(T1) = (P2)(V2)/(n2)(T2)
I concluded (perhaps incorrectly) that the n's and T's cancel out since there is no change at all.
I then calculated (again perhaps incorrectly) that the V2 was equal to 143.84 mL.
Can someone check my answer or tell me how to solve it? Thank you in advance!
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P1V1=P2V2 Correct, you do not need n or T for this problem.
1 atm = 760mmHg
Convert:
P1= 0.9736atm
V1 = 0.223L
*volume in these problems should always be in Liters
Put it all into the equation...
(0.97)(0.223L)=(1.51atm)(xL)
.217=x1.51
x = .1437L = V2
1 atm = 760mmHg
Convert:
P1= 0.9736atm
V1 = 0.223L
*volume in these problems should always be in Liters
Put it all into the equation...
(0.97)(0.223L)=(1.51atm)(xL)
.217=x1.51
x = .1437L = V2
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Why does volume always have to be Litres ??
Whatever volume units are used, no conversion is necessary unless asked for.
Whatever volume units are used, no conversion is necessary unless asked for.
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