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pochemuha
2 years ago
5

Why is it usually warmer at Earth’s equator than at its poles?

Chemistry
1 answer:
MissTica2 years ago
8 0

Answer:

the equator is closer to the sun

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The freezing point of 42.19 g of a pure solvent is measured to be 43.17 ºC. When 2.03 g of an unknown solute (assume the van 't
vovikov84 [41]

Answer:

The molality of the solution is 0.3716 mol/kg

The number of moles of solute is 0.0157 mol

The molecular weight of the solute is 129.30 g/mol

The molar mass of the solute is 129.32 g/mol

Explanation:

m (molality of the solution) = ∆T/Kf = (43.17 - 40.32)/7.67 = 0.3716 mol/kg

Number of moles of solute = molality × mass of solvent in kilogram = 0.3716 × 0.04219 = 0.0157 mol

Molecular weight of solute = mass/number of moles = 2.03/0.0157 = 129.3 g/mol

When Kf = 7.66 °C.kg/mol

Molar mass = 2.03 ÷ (2.85/7.66 × 0.04219) = 129.32 g/mol

4 0
3 years ago
Calculate the half-life of different radioactive sources.
otez555 [7]
The rate at which a radioactive<span> isotope decays is measured in </span>half-life. The termhalf-life<span> is defined as the time it takes for one-</span>half<span> of the atoms of a </span>radioactive material<span> to disintegrate. </span>Half-lives<span> for </span>various radioisotopes<span> can range from a few microseconds to billions of years.
</span>.
back at it again with that answer
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zane
7 0
3 years ago
What mass of barium chloride, BaCL2, is required to completely precipitate the barium sulfate from 35.0 ml of 0.200 m h2so4?
faltersainse [42]
The balanced equation would be (1)BaCl2 + (1)H2SO4 --> (1)BaSO4 + (2)HCl2
Then you should know that the coefficients stand for moles.
The thing is I'm not sure if H2SO4 is 35 ml or .200 m. 
Also, is this topic stoichiometry?
5 0
3 years ago
Does anybody know how to do q4. Please show working out thanks.
insens350 [35]

Answer:

% purity of limestone = 96.53%

Explanation:

Question (4).

Weight of impure CaCO₃ = 25.9 g

Molecular weight of CaCO₃ = 40 + 12 + 3(16)

                                              = 100 g per mole

We know at S.T.P. number of moles of CO₂ = 1 and volume = 22.4 liters

From the given reaction, 1 mole of CaCO₃ reacts with 1 mole or 22.4 liters of

CO₂.

∵ 22.4 liters of CO₂ was produced from CaCO3 = 100 g

∴ 1 liter of CO₂ will be produced by CaCO₃ = \frac{100}{22.4}

∴ 5.6 liters of CO₂ will be produced by CaCO₃ = \frac{100\times 5.6}{22.4}

                                                                              = 25 g

Therefore, % purity of CaCO₃ = \frac{\text{Weight calculated}}{{\text{Weight given}}}\times 100

                                                 = \frac{25}{25.9}\times 100

                                                 = 96.53 %

7 0
3 years ago
96.0 g. of a gas occupies 48.0 L at 700.0 mm Hg and 20.0 °C. What is its molecular weight?
g100num [7]

Answer:

I hope this helps 52.2 g/mol

Explanation:

1) Solve for the moles using PV = nRT:

n = PV / RT

n = [(700.0 mmHg / 760.0 mmHg atm¯1) (48.0 L)] / [(0.08206 L atm mol¯1 K¯1) (293.0 K)]

n = 1.8388 mol

2) Divide the grams given (96.0) by the moles just calculated above:

96.0 g / 1.8388 mol = 52.2 g/mol

7 0
2 years ago
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