Answer:
14.7°C
Explanation:
Q = m·ΔT·c
ΔT = 
ΔT =
= 1320 J / ((230 g) * (.39 J/g°C)
ΔT = 14.7 °C
Answer:
The answer to your question is 8.21 g of H₂O
Explanation:
Data
mas of water = ?
mass of hydrogen = 4.6 g
mass of oxygen = 7.3 g
Balanced chemical reaction
2H₂ + O₂ ⇒ 2H₂O
Process
1.- Calculate the atomic mass of the reactants
Hydrogen = 4 x 1 = 4 g
Oxygen = 16 x 2 = 32 g
2.- Calculate the limiting reactant
Theoretical yield = H₂/O₂ = 4 / 32 = 0.125
Experimental yield = H₂/ O₂ = 4.6/7.3 = 0.630
From the results, we conclude that the limiting reactant is Oxygen because the experimental yield was higher than the theoretical yield.
3.- Calculate the mass of water
32 g of O₂ ---------------- 36 g of water
7.3 g of O₂ --------------- x
x = (7.3 x 36) / 32
x = 262.8 / 32
x = 8.21 g of H₂O
Answer:
56160grams
Explanation:
First, we need to convert the number of molecules of magnesium chloride (MgCl2) into moles by dividing by Avagadro's number (6.02 × 10^23 molecules)
n = nA ÷ 6.02 × 10^23
n = 14.07 × 10^26 ÷ 6.02 × 10^23
n = 14.07/6.02 × 10^(26-23)
n = 2.34 × 10^3 moles of MgCl2
The balanced reaction given in the question is as follows:
Mg + 2HCl → MgCl2 + H2
If 1 mole of Mg produced 1 mole of MgCl2
Then, 2.34 × 10^3 moles of Mg will also produce 2.34 × 10^3 moles of MgCl2.
Using mole = mass ÷ molar mass (MM)
Molar mass of Mg = 24g/mol
mass = mole × MM
mass = 2.34 × 10^3 × 24
mass = 56.16 × 10^3
mass = 56160grams.
Number 6 is D the mitochondrion
