Answer: 2.7 grams
Explanation:
According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.
Given: mass of sodium hydrogen carbonate = 3.4 g
mass of acetic acid = 10.9 g
Mass of reactants = mass of sodium hydrogen carbonate+ mass of acetic acid = 3.4 + 10.9= 14.3 g
Mass of reactants = Mass of products in reaction vessel + mass of carbon dioxide (as it escapes)
Mass of carbon dioxide = 14.3 - 11.6 =2.7 g
Thus the mass of carbon dioxide released during the reaction is 2.7 grams.
Answer:
V₂ = 568.9 mL
Explanation:
Given data:
Volume of gas = 550 mL
Pressure of a gas = 960 mmHg
Temperature = 200.0°C ( 200+273 = 473 K)
Final volume = ?
Final pressure = 830 mmHg
Final temperature = 150°C (150+273 = 423 K)
Solution:
Formula:
P₁V₁/T₁ = P₂V₂/T₂
P₁ = Initial pressure
V₁ = Initial volume
T₁ = Initial temperature
P₂ = Final pressure
V₂ = Final volume
T₂ = Final temperature
Solution:
V₂ = P₁V₁ T₂/ T₁ P₂
V₂ = 960 mmHg × 550 mL × 423 K / 473 K ×830 mmHg
V₂ = 223344000 mL / 392590
V₂ = 568.9 mL
Answer:
8×10^(-3) mol/L
Explanation:
The formula for finding the hydrogen ion concentration is...
[H⁺] = 10^-ph
[H⁺] = 10^(-2.1)
[H⁺] = 0.00794...mol/L = 8×10^(-3) mol/L
The answer is to 1 significant digit because the pH has one decimal place.
Answer:
i believe it is number #3
Explanation:
hope this helps
Answer:
Molecular Formula = C₆H₁₂O₆
Solution:
Molecular formula is calculated by using following formula,
Molecular Formula = n × Empirical Formula ---- (1)
Also, n is given as,
n = Molecular Weight / Empirical Formula Weight
Molecular Weight = 180.2 g.mol⁻¹
Empirical Formula Weight = 12 (C) + 2 (H₂) + 16 (O) = 30 g.mol⁻¹
Son
n = 180.2 g.mol⁻¹ ÷ 30 g.mol⁻¹
n = 6
Putting Empirical Formula and value of "n" in equation 1,
Molecular Formula = 6 × CH₂O
Molecular Formula = C₆H₁₂O₆
