Answer:
Q = 52668 J
Explanation:
Given data:
Amount of heat required = ?
Mass of water = 350 g
Initial temperature = 20°C
Final temperature = 56°C
Specific heat capacity of water = 4.18 J/g°C
Solution:
Formula:
Q = m.c. ΔT
Q = amount of heat absorbed or released
m = mass of given substance
c = specific heat capacity of substance
ΔT = change in temperature
ΔT = 56°C - 20°C
ΔT = 36°C
Q = 350 g× 4.18 J/g°C ×36°C
Q = 52668 J
Answer: 24.13 g Cu
Explanation:
<u>Given for this question:</u>
M of CuO = 30 g
m of CuO = 79.5 g/mol
Number of moles of CuO = (given mass ÷ molar mass) = (30 ÷ 79.5) mol
= 0.38 mol
The max number of CuO (s) that can be produced by the reaction of excess methane can be solved with this reaction:
CuO(s) + CH4(l) ------> H2O(l) + Cu(s) + CO2(g)
The balanced equation can be obtained by placing coefficients as needed and making sure the number of atoms of each element on the reactant side is equal to the number of atoms of each element on the product side
4CuO(s) + CH4(l) ----> 2H2O(l) + 4Cu(s) + CO2(g)
From the stoichiometry of the balanced equation:
4 moles of CuO gives 4 moles of Cu
1 mole of CuO gives 1 mol of Cu
0.38 mol of CuO gives 0.38 mol of Cu
Therefore, the grams of Cu that can be produced = 0.38 × molar mass of Cu
= 0.38 × 63.5 g
= 24.13 grams
Therefore, 24.13 grams of copper could be produced by the reaction of 30.0 of copper oxide with excess methane
The combined-gas law relates which temperature, pressure and volume.
Temperature=T
Pressure=P
Volume=V
<span>(P₁*V₁) / T₁=(P₂*V₂) / T₂
D. Temperature, pressuere and volume.</span>
Answer:
Explanation:
We can use Dalton's Law of Partial Pressures:
Each gas in a mixture of gases equals its pressure independently of the other gases
Answer: 1
Explanation: coarse adjustment
