0.309g
Explanation:
Mass of evaporating dish = 6.251g
Mass of evaporating dish and sample of hydrate = 16.864g
solving for mass of hydrate before heating;
Mass of hydrate =
mass of evaporating dish and sample of hydrate - mass of evaporating dish;
Mass of hydrate before heating = 16.864g - 6.251g = 10.613g
Upon heating ;
Mass of hydrate plus dish = 11.3g
Unknown:
number of moles of water removed from the hydrate = ?
We need to find the mass of water removed from the hydrate;
Mass of hydrate after heating =mass of hydrate plus dish after heating - mass of evaporating dish
mass of hydrate after heating = 11.3g - 6.251g = 5.049g
Mass of water lost = Mass of hydrate before heating - mass of hydrate after heating
= 10.613g - 5.049g
= 5.564g
Number of moles of water = 
number of moles of water = 0.309moles
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Number of moles brainly.com/question/13064292
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2H2 + O2 ---->2H2O
number of moles in reaction 2 mol 1 mol 2 mol
number of liters in the reaction 2*22.4 L 1*22.4 L 2*22.4L
We can see that volumes of the gases are proportional to coefficients in the reaction ( if gases are under the same conditions), so we can write
2H2 + O2 ---->2H2O
2 L 1 L 2 L
given 40 L ( 25 L) 40 L
We can see that we have excess of O2,
because if 2 L H2 are needed 1 L O2, then 40 L of H2 are needed 20 L O2.
So, limiting reactant is H2, and we will need to calculate Volume of H2O using H2.
2L H2 give 2L H2O(gas), so 40 L H2 give 40 L H2O.
Answer:
16.5 atm
Explanation:
<em>A mixture of He, N₂, and Ar has a pressure of 24.1 atm at 28.0 °C. If the partial pressure of He is 3013 torr and that of Ar is 2737 mm Hg, what is the partial pressure of N₂?</em>
The total pressure of a gaseous mixture is equal to the sum of the partial pressures.
P = pHe + pN₂ + pAr
pN₂ = P - pHe - pAr [1]
We need to express pHe and pAr in atm.


From [1],
pN₂ = 24.1 atm - 3.96 atm - 3.60 atm = 16.5 atm
Answer:
yes
Explanation:
this is because the formula equation shows the details on how they solved the equation