Answer:
Explanation:
Vaporization Equation => Q = m·ΔHv
m = 0.5Kg water = 500g water
ΔHv = Heat of vaporization = 540 calories/gram
∴Q = 500g x 540cal/g = 270,000 calories x 4.184 joules/cal = 1,129,680 joules = 1130 Kilojoules (3 sig. figs.)
Answer:
a. 6 mol of oxygen
b. 10 mol of iron(III)oxide
Explanation:
Use mole concept.
That is not a question/problem and makes no sense whatsoever
Explanation:
The given data is as follows.
= 98.70 kPa = 98700 Pa,
T = 
= (30 + 273) K = 303 K
height (h) = 30 mm = 0.03 m (as 1 m = 100 mm)
Density = 13.534 g/mL = 
= 13534 
The relation between pressure and atmospheric pressure is as follows.
P = 
Putting the given values into the above formula as follows.
P =
= 
= 102683.05 Pa
= 102.68 kPa
thus, we can conclude that the pressure of the given methane gas is 102.68 kPa.
The correct balanced chemical equation which occur when methane burn in oxygen gas is
CH4 + 2O2 --> 2H2O +CO2 (answer D)
when methane is burned in presence of oxygen gas it produces carbon(IV) oxide and water and energy,that is 1 mole of CH4 reacted with 2 moles of O2 to form 2 moles of water and 1 mole of CO2 and enegy. This energy make the methane to be used as fuel.
