Acids are ionic compounds (a compound with a positive or negative charge) that break apart in water to form hydrogen ion (H+). Characteristics of acid: Acid taste sour. Acids also react strongly to metals, generally with the evolution of hydrogen gas (Eg: Zn + HCI). Also strong acids are dangerous and can burn your skin off. Acids change litmus red. Acids become less acidic when mixed with bases. An acid has Ph scale of under 7.
Answer:
13.44dm^3
Explanation:
To calculate this we first need to know the number of mole produced. We will first need to balance the equation to know the theoretical mole ratio.
C2H6 (g) + 3.5O2 (g) → 2CO2 (g) + 3H2O (g)
From the balanced equation, we can deduce that one mole of ethane yielded 2 moles of carbon iv oxide. We use this information to calculate the actual number of moles yielded.
24g were reacted. Now to know the number of moles reacted, we simply divide the mass by the molar mass. The molar mass of ethane is 2(12) +6(1)= 40g/mol
The number of moles is thus 24/40 = 0.6 moles
Like we said earlier, one mole yielded 2 moles of carbon iv oxide, hence, 0.6 moles will yield 0.6 * 2 = 0.12 moles of carbon iv oxide.
Now, at stp, one mole of a gas occupies a volume of 22.4dm^3 thus, 0.6 mole will occupy 0.6 * 22.4 = 13.44dm^3
Answer:
3.1 mol
Step-by-step explanation:
The balanced equation is
CaCl₂ + 2AgNO₃ ⟶ Ca(NO₃)₂ + 2AgCl
You want to convert moles of AgNO₃ to moles of CaCl₂.
The molar ratio is 2 mol AgNO₃:1 mol CaCl₂
Moles of CaCl₂ = 6.2 mol AgNO₃ × (1 mol CaCl₂/2 mol AgNO₃)
Moles of CaCl₂ = 3.1 mol CaCl₂
The reaction will require 3.1 mol of CaCl₂.
Answer:
Mass = 7.2 g
Explanation:
Given data:
Mass of water produced = ?
Mass of oxygen = 7.8 g
Solution:
Chemical equation:
2H₂ + O₂ → 2H₂O
Number of moles of oxygen:
Number of moles = mass/ molar mass
Number of moles = 7.8 g/ 32 g/mol
Number of moles = 0.2 mol
Now we will compare the moles of water with oxygen.
O₂ : H₂O
1 : 2
0.2 : 2×0.2 = 0.4 mol
Mass of water:
Mass = number of moles × number of moles
Mass = 0.4 mol × 18 g/mol
Mass = 7.2 g
