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1 year ago

The molar mass of an imaginary molecule is is 93.89 g/mol. Determine its density at STP.

Chemistry

1 answer:

Igoryamba1 year ago

3 0

Answer:

Density = 4.191 gm/L

Explanation:

Given:

Molar mass = 93.89 g/mol

Volume(Missing) = 22.4 L (Approx)

Find:

Density at STP

Computation:

Density = Mass/Volume

Density = 93.89 / 22.4

Density = 4.191 gm/L

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Material A has a small latent heat of fusion. Material B has a large heat of fusion. Which of the following statements is true?

Olin [163]

The correct answer would be the first option. Material A having a smaller latent heat of fusion would mean that it will take only less energy to phase change into the liquid phase. Latent of heat of fusion is the amount of energy needed of a substance to phase change from solid to liquid or liquid to solid.

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2 years ago

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When 64.0 g of methanol (CHOH) is burned, 1454 kJ of energy is produced. What is the heat of combustion for methanol?

andreev551 [17]

The heat of combustion for methanol is 727 kj/mol

<em><u>calculation</u></em>

calculate the moles of methanol (CH3OH)

moles = mass/molar mass

molar mass of methanol = 12 +( 1 x3) +16 + 1= 32 g /mol

moles is therefore= 64.0 g / 32 g/mol = 2 moles

Heat of combustion is therefore = 1454 Kj / 2 moles = 727 Kj/mol

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2 years ago

II. Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 3.86 g of magnesium ribbo

Leto [7]

Answer:

$Excess=3.53g$

Explanation:

Hello,

In this case, the undergoing chemical reaction is:

$2Mg(s)+O_2(g) \rightarrow 2MgO(s)$

Next, we identify the limiting reactant by computing the moles of magnesium oxide yielded by 3.86 g of magnesium and 155 mL of oxygen at the given conditions via their 2:1:2 mole ratios and the ideal gas equation:

$n_{MnO}^{by \ Mg}=3.86gMg*\frac{1molMg}{24.3gMg}*\frac{2molMgO}{2molMg} =0.159molMgO\\\\n_{MnO}^{by \ O_2}=\frac{1atm*0.155L}{0.082\frac{atm*L}{molO_2*K}*275K} *\frac{2mol MgO}{1molO_2} =0.0137molMgO$

It means that the limiting reactant is the oxygen as it yields the smallest amount of magnesium oxide. Next, we compute the mass of magnesium consumed the oxygen only:

$m_{Mg}^{consumed}=0.0137molMgO*\frac{2molMg}{2molMgO} *\frac{24.3gMg}{1molMg} =0.334gMg$

Thus, the mass in excess is:

$Excess=3.86g-0.334g\\\\Excess=3.53g$

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2 years ago

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LiRa [457]

Answer:

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2 years ago

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Bond [772]

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b. Double displacement reaction is one in which exchange of ions take place.

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c. Decomposition is a type of chemical reaction in which one reactant gives two or more than two products.

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1 year ago