If 0.0469 g of mg metal reacted with hydrochloric acid completely, temperature is 21.0 c barometric pressure is 759.0 mm hg, and the product was collected by volume by water displacement; how much volume of gases would be measured in ml? show your work!
a) what is the temperature in kelvin?
b) what is partial pressure due to water vapor at 21.0 c?
c) what is partial pressure of the hydrogen gas, ph2 (in atm)? *remember dalton's law of partial pressures for a "wet" gas*
d) what is moles of hydrogen gas created in moles?
e) what is the ideal gas law constant, r (in atm-l/mole- k) ?
f) what is the working equation for volume ( using pv= nrt)
g) what is the volume of gases in ml?

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explanation:

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2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

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