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den301095 [7]
3 years ago
9

Which condition applies when water boils at 100°c? air pressure equals a specific value (101.3 kpa) air pressure is less than it

s value at the triple point of water air pressure is zero, as in a vacuum vapor pressure is zero
Chemistry
2 answers:
Alinara [238K]3 years ago
8 0
Water normally boils when the vapor pressure of water is equal to the external pressure. That is, at 100 degree Celsius, the external vapor will be 101.3 kpa. The correct answer is A.
FrozenT [24]3 years ago
4 0

The correct answer is air pressure equals a specific value(101.3 kpa)

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How many grams of oxygen (O) are present in 0.0207 moles of Ca(HCO 3) 2
Zolol [24]

Answer:

1.99grams

Explanation:

- First, we need to calculate the molar mass of the compound: Ca(HCO3)2

Ca = 40g/mol, H = 1g/mol, C = 12g/mol, O = 16g/mol

Hence, Ca(HCO3)2

= 40 + {1 + 12 + 16(3)}2

= 40 + {13 + 48}2

= 40 + {61}2

= 40 + 122

= 162g/mol

Molar mass of Ca(HCO3)2 = 162g/mol

- Next, we calculate the mass of oxygen in one mole of the compound, Ca(HCO3)2.

Oxygen = {16(3)}2

= 48 × 2

= 96g of Oxygen

- Next, we calculate the percentage composition of oxygen by mass by dividing the mass of oxygen in the compound by the molar mass of the compound i.e.

% composition of O = 96/162 × 100

= 0.5926 × 100

= 59.26%.

- The number of moles of the compound, Ca(HCO3)2, must be converted to mass by using the formula; mole = mass/molar mass

0.0207 = mass/162

Mass = 162 × 0.0207

Mass = 3.353grams

However, in every gram of Ca(HCO3)2, there is 0.5926 g of oxygen

Hence, in 3.353grams of Ca(HCO3)2, there will be;

0.5926 × 3.353

= 1.986

= 1.99grams.

Therefore, there is 1.99grams of Oxygen in 0.0207 moles (3.353g) of Ca(HCO3)2.

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