Answer:
Explanation:
Hello,
In this case, the undergoing chemical reaction is:
Next, we compute the reacting moles of each reactants:
Then, as magnesium and hydrohloric acid are in a 1:2 molar ratio 0.153 moles of magnesium will completely react with 0.306 moles of hydrochloric acid yet we only have 0.144 moles, therefore, limiting reactant is hydrochloric acid. Thus, we compute the produced moles of hydrogen:
Finally, we use the ideal gas equation with T=298K and 1atm (STP conditions) to compute the liters of hydrogen gas:
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Answer:
Explanation:
Considering,
Using ideal gas equation as:
where,
P is the pressure = 760 mmHg
V is the volume = 100.0 mL = 0.1 L
m is the mass of the gas = 0.193 g
M is the molar mass of the gas = ?
Temperature = 17 °C
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T = (17 + 273.15) K = 290.15 K
R is Gas constant having value = 62.36367 L. mmHg/K. mol
Applying the values as:-
M = 45.95 g/mol
This mass corresponds to . Hence, the gas must be .
This is a simple chemical change due to what it produces and how it is added together. Hope this helps.
1.
2.Unconformity
3. Folding
4. Law of superposition
