Electrical energy can be used to separate water into O2(g) and H2(g). In one demonstration of this reaction, 17.00 mL of H2 are collected over water at 25°C. Atmospheric pressure is 741.0 mmHg. How many grams of hydrogen are collected?
the weight of hydrogen is calculated by gas law principle.
PV = nRT
where
P + Pressure in HG mm,
V = volume in lit here 17 ml
T =temperature in kelvin here 25C.
R = constant of ideal gas
n = no of mole of hydrogen
the answer is calculated by putting the value of respective parameters
= .000677 mole
so multiplying this with hydrogen mol wt 2 = 0.00135 gm hydrogen
Electrical energy can be used to separate water into O2(g) and H2(g). In one demonstration of...
Electrical energy can be used to separate water into O2(g) and H2(g). In one demonstration of this reaction, 17.00 mL of H2 are collected over water at 25°C. Atmospheric pressure is 741.0 mmHg. How many grams of H2 are collected?
Electrical energy can be used to separate water into O2(g) and H2(g). In one demonstration of this reaction, 17.00 mL of H2 are collected over water at 25°C. Atmospheric pressure is 741.0 mmHg. How many grams of H2 are collected?
1st attempt di See Periodic Table See Hint In one demonstration of this reaction, 32.00 mL of H2 are collected over water at 25°C. Atmospheric pressure is 759.0 mmHg. How many grams of H2 are collected? g Hydrogen MacBo esc Fl F4 F5 F6 4
2 Calculate the pressure of the Hydrogen gas collected. Water temperature was 23.0 ° C and the atmospheric pressure was 741.0 mmHg. (Hint the density of Mercury is 13.6 g/mL) H2 gas collected over water 220. mm H20 RT
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homework :)
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