What happens to ionization energy as you go across a period from left to right

A chemical reaction that is expected to form 325.0 gof product only forms 123.8 g of product. What is the percent yield of this

Tasya [4]

Answer:

$\boxed {\boxed {\sf A. \ 38.1 \%}}$

Explanation:

Percent yield is the ratio of the amount actually produced to how much could theoretically be produced. It is found using this formula:

$\% \ yield = \frac{actual \ yield}{theoretical \ yield} *100$

For this reaction, the theoretical or expected yield is 325.0 grams. The actual yield is 123.8 grams.

$\% \ yield = \frac{ 123.8 \ g }{325.0 \ g }*100$

Divide.

$\% \ yield = 0.380923077 *100$

$\% \ yield = 38.0923077$

Round to the nearest hundredth. The 9 in the hundredth place tells us to round the 0 to a 1 .

$\% \ yield \approx 38.1$

The percent yield is about 38.1%

5 0

2 years ago

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The specific heat capacity of a pure substance can be found by dividing the heat needed to change the temperature of a sample of

kupik [55]

Answer:

See below

Explanation:

ΔQ = m c T ΔQ = heat required(J) m = mass (g) T = C° temp change

c = heat capacity in J/g-C

4 0

2 years ago

If two identical atoms are bonded together, what kind of molecule is formed?

AlekseyPX

Answer:

C. A linear, nonpolar molecule

Explanation:

Molecules which are alike usually have the same degree of pull which results in them sharing electrons. This sharing of electrons is known as the molecules exhibiting Covalent bonding between them.

The equal pull also results in the cancelling out of electrons and favoring non polar bonds due to the absence of free electrons which would have been able to interact with H2O in a polar binding system.

6 0

3 years ago

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What is the number of electronsin hydrogen

tino4ka555 [31]

Answer:

There's only one electron in hydrogen.

4 0

2 years ago

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CHEM HELP ASAP!! What mass of H2 would be needed to produce 208 kg of methanol?

Eddi Din [679]

So if we use the equation:

$CO+2H_{2}$ → $CH_{3}OH$

We can then determine the amount of $H_{2}$ needed to produce 208 kg of methanol.

So let's find out how many moles of methanol 208 kg is:

Methanol molar weight = 32.041g/mol

So then we can solve for moles of methanol:

$208kg*\frac{1,000g}{1kg} *\frac{1mol}{32.041g} =6,491.68mol$

So now that we have the amount of moles produced, we can use the molar ratio (from the balanced equation) of hydrogen and methanol. This ratio is 2:1 hydrogen:methanol.

Therefore, we can set up a proportion to solve for the moles of hydrogen needed:

$\frac{2}{1} =\frac{x}{6,491.68}$

$x=12,983.36mol$

So now that we have the number of moles of $H_{2}$ that are produced, we can then use the molar weight of hydrogen to solve for the mass that is needed:

$12,983.36mol*\frac{2.016g}{1mol} =26,174.45g_H_{2}$

Therefore, the amount of diatomic hydrogen ( $H_{2}$ ) that is needed to produce 208kg of methanol is $2.62x10^{4}$ g.

3 0

3 years ago