Given the balanced equation representing a reaction: Zn(s) + 2HCl(aq) - H2(g) + ZnCl2(aq)
Which set of reaction conditions produces H2(g) at the fastest rate?
A.
a 1.0-g lump of Zn(s) in 50. mL of 0.5 M HCl(aq) at 20.°C
B.
a 1.0-g lump of Zn(s) in 50. mL of 0.5 M HCl(aq) at 30.°C
C.
1.0 g of powdered Zn(s) in 50. mL of 1.0 M HCl(aq) at 20. °C
D
1.0 g of powdered Zn(s) in 50. mL of 1.0 M HCl(aq) at 30.°C

D  1.0 g of powdered Zn(s) in 50. mL of 1.0 M HCl(aq) at 30.°C

Explanation:

There are several factors affecting and controlling the rate of chemical reactions.

Some of which are applicable in resolving this problem is the nature of the reactants and their concentration. Also, the temperature of the reaction is also very important.

take a better picture and ill do it

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.