All categories

3 years ago

How much heat is released when you condense 93.9 g of water vapor? Show work please ❤️

Chemistry

1 answer:

sammy [17]3 years ago

7 0

Answer:

211.9 J

Explanation:

The molecules of water release heat during the transition of water vapor to liquid water, but the temperature of the water does not change with it.

The amount of heat released can be represented by the formula:

$Q=mL_e$

where $Q$ = heat energy, $m$ = mass of water and $L$ = latent heat of evaporation.

The latent heat of evaporation for water is $L=2257 kJ/kg$ and the mass of the water is $m=93.9 g=0.0939 kg$ .

The amount of heat released in this process is:

$Q=mL_e = (0.0939kg)(2257 kJ/kg)=$ 211.9 J

You might be interested in

1pt Which statement best describes the relationship between the system and the surroundings?

Firlakuza [10]

Answer:

Hi how are you doing today Jasmine

4 0

3 years ago

How do the process of crabon cycle contribute to climate change.

bonufazy [111]

Explanation:

Carbon that is a part of rocks and fossil fuels like oil, coal, and natural gas may be held away from the rest of the carbon cycle for a long time. These changes add more greenhouse gases in our atmosphere and this causes climate change.

3 0

3 years ago

The relative abundances of the stable isotopes of the elements are not entirely constant. For example, in some geologic samples

Mrac [35]

Answer: The other isotope is $_{37}^{87}\textrm{Rb}$

Explanation:

Beta decay is defined as the decay process in which a neutron gets converted to a proton and an electron.

In this decay process, beta particle is emitted. The emitted particle carries a charge of -1 units and has a mass of 0 units. The released beta particle is also known as electron.

The general equation for the beta decay process follows:

$_Z^A\textrm{X}\rightarrow _{Z+1}^A\textrm{Y}+_{-1}^0\beta$

The chemical equation for the beta decay of an isotope that produces Sr-87 isotope follows:

$_{37}^{87}\textrm{Rb}\rightarrow _{38}^{87}\textrm{Sr}+_{-1}^0\beta$

The isotope that undergoes beta decay to form Strontium-87 isotope is Rubidium-87

Hence, the other isotope is $_{37}^{87}\textrm{Rb}$

4 0

3 years ago

A key step in the extraction of iron from its ore isFeO(s) + CO(g) ⇄ Fe(s) + CO₂(g) Kp = 0.403 at 1000°CThis step occurs in the

Kisachek [45]

A key step in the extraction of iron from its ore isFeO(s) + CO(g) ⇄ Fe(s) + CO₂(g) Kp = 0.403 at 1000°CThis step occurs in the 700°C to 1200°C zone within a blast furnace. the partial pressure of CO2 at equilibrium is 1.58 atm.

The complete reaction of the problem, for better illustration, is

FeO(s) + CO(g) <--> Fe(s) + CO2(g)

The double-tailed arrow signifies that the reaction is in a dynamic chemical equilibrium. When the system is in equilibrium, the forward and the backward reaction rates have an equal ratio of Kp = 0.403 at 1000°C. The formula for Kp is

Kp = [partial pressure of products]/[partial pressure of reactants]

So, first, let's find the partial pressure of the compounds in the reaction.

FeO(s) + CO(g) <--> Fe(s) + CO2(g)

Initial x 1.58 0 0

Change -1.58 -1.58 +1.58 +1.58

------------------------------------------------------------------

Equilbrium x-1.58 0 1.58 1.58

Kp = [(1.58)(1.58)]/[(x-1.58)] = 0.403

x = 7.77 atm (this is the amount of excess FeO)

Therefore, the partial pressure of CO2 at equilibrium is 1.58 atm. There is no more CO because it has been consumed due to excess FeO.

To know more about partial pressure of CO2 at equilibrium

brainly.com/question/16022760

#SPJ4

6 0

1 year ago

What mass of magnesium oxide is formed when 48.62g of magnesium is reacted with excess oxygen?

marin [14]

Answer: -

81.03 g magnesium oxide is formed when 48.62g of magnesium is reacted with excess oxygen

Explanation: -

Atomic mass of Mg = 24 g

Molar mass of MgO = 24 x 1 + 16 x 1

= 40 g

The balanced chemical equation for this reaction is

2 Mg + O₂ → 2MgO

From the balanced chemical equation we see

2 mol of Mg gives 2 mol of MgO.

2 x 24 g of Mg gives 2 x 40g of MgO.

48.62 g of Mg gives $\frac{2 x 40 g MgO}{2 x 24 g Mg}$ x Mg

= 81.03g of MgO

5 0

3 years ago