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OleMash [197]
2 years ago
9

A 36-gram sample of water has an initial temperature of 22°c. After the sample absorbs 1200 joules of heat energy, the final tem

perature of the sample is.
Chemistry
1 answer:
professor190 [17]2 years ago
7 0

Answer:

≈29.94 [°C].

Explanation:

all the details are in the attachment, the answer is underlined with orange colour.

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Calculate the mass of excess reagent remaining at the end of the reaction in which 90.0 g of SO2 are mixed with 100.0 g of O2
Radda [10]
We have to first write a balanced equation.
so2 + o2 -> so3

this is not balanced though. we have 3 oxygen on right and 4 on left
2so2 + o2 -> 2so3

now it is same on both sides. we have to figure out which is limiting reagent with the given amounts of reagents. we do this by comparing the ratio between them in terms of moles. we see that so2 has a coefficient of 2 and o2 has none which implies 1 and so3 has 2. this means that for every 2 moles of so2 reacting with 1 mole of o2, we get 2 moles of so3.

lets convert the given values to moles. to do this we know that molecular weight is measured in grams per mole. we are given grams and need to cancel out the grams to get moles. so the molecular weight:
so2 =32.1 + 2 * 16 = 64.1 g/mol
o2 = 2 * 16 = 32 g/mol
so3 = 32.1 + 3 * 16 = 80.1 g/mol

now to convert 90 g of 2so2 under ideal conditions.
90g / 64.1g/mol = 1.404 moles

convert this amount of moles of so2 to moles of o2. we have 2 moles of so2 to 1 of o2
1.404moles so2 / 2 moles so2 * 1 mole o2= 0.702 moles o2

so we see under ideal conditions that 90g of so2 would react with .702g of o2. lets see how many we actually have with 100g of o2
100g / 32g/mol =3.16 mol.

so we have a lot more o2 than needed. we are looking for how much is left in grams. we have to figure out how much was used. to do this convert our ideal moles of o2 into grams.
.702 moles o2 * 32g/mol = 22.5g o2

so what we startrd with (100g) minus what we needed (22.5g) is what we have left
100 - 22.5 = 77.5g o2
6 0
3 years ago
At 25°c, the vapor in equilibrium with a solution containing carbon disulfide and acetonitrile has a total pressure of 250. torr
Sonbull [250]
For this question, we apply the Raoult's Law. The formula is written below:

P = P*x
where
P is the partial pressure
P* is the vapor pressure of the pure solvent
x is the mole fraction

The partial pressure is solved as follows:
P = Total P*x = (250 torr)(0.857) = 214.25 torr
Hence,
214.25 = (361 torr)(x)
<em>x = 0.593 or 59.3%</em>
8 0
3 years ago
The structure of oxides of highly electronegative element is ​
e-lub [12.9K]
<h2>Hey there! </h2>

<h3>Your answer is:</h3>

<h3>ns^2np^5</h3>

<h3>The most electronegative element is Fluorine. It is a halogen group element. Its outer shell electronic configuration is ns^2np^5</h3>

<h2>Hope it help you </h2>

8 0
3 years ago
Synthesis of acetic acid from acetylene
devlian [24]
Acetylene can be converted into acetic acid in 2 steps:

1. reaction of acetylene with water (in the presence of sulphuric acid, and mercuric sulphate as catalysts) to produce acetaldehyde.

2. acetaldehyde is then oxidized (with potassium dichromate for example) to produce acetic acid.

this overall reaction is given by the following equation:


3 0
3 years ago
Methylamine has a vapor pressure of 344torr at −25∘C and a boiling point of −6.4∘C . Find ΔHvap for methylamine.
hram777 [196]
The Clausius-Clapeyron equation:
ln(P₁/P₂) = ΔH/R * (1/T₂ - 1/T₁)

-25 °C = 248 K and pressure is 344 torr
-6.4 °C = 266.6 K and pressure is 760 torr (atmospheric)

Using the equation:

ln(760/344) = ΔH/62.364 * (1/248 - 1/266.6)
ΔH = 175.7 kJ/mol
6 0
3 years ago
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