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2 years ago

What could you do to make yeast dough rise more slowly?

Chemistry

2 answers:

Nitella [24]2 years ago

6 0

Answer:

So, if you want to slow down rise without much testing, controlling temperature—allow for a slow rise in the refrigerator or add cold liquid to the dough instead of the usually recommended warm liquid—is the more surefire method. Therefore, your answer should be D.

Explanation:

olganol [36]2 years ago

3 0

Answer:

d. Reduce the temperature

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Explanation:

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2 years ago

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2 years ago

Name two properties that make solutions different from colloids.

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1 year ago

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Oxalic acid can remove rust (Fe2O3) caused by bathtub rings according to the reaction Fe2O3(s) - 6H2C2O4(aq) rightarrow 2Fe(C2O4

Katena32 [7]

Answer: The mass of rust that can be removed is 1.597 grams

Explanation:

To calculate the number of moles for given molarity, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}$ .....(1)

Molarity of oxalic acid solution = 0.1255 M

Volume of solution = $6.00\times 10^2mL$ = 600 mL = 0.600 L (Conversion factor: 1 L = 1000 mL)

Putting values in equation 1, we get:

$0.100M=\frac{\text{Moles of oxalic acid}}{0.600L}\\\\\text{Moles of oxalic acid}=(0.100mol/L\times 0.600L)=0.06mol$

For the given chemical reaction:

$Fe_2O_3(s)+6H_2C_2O_4(aq.)\rightarrow 2Fe(C_2O_4)_3^{3-}(aq.)+3H_2O(l)+6H^+(aq.)$

By Stoichiometry of the reaction:

6 moles of oxalic acid reacts with 1 mole of ferric oxide (rust)

So, 0.06 moles of oxalic acid will react with = $\frac{1}{6}\times 0.06=0.01mol$ of ferric oxide (rust)

To calculate the mass of rust for given number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Molar mass of rust (ferric oxide) = 159.7 g/mol

Moles of rust = 0.01 moles

Putting values in above equation, we get:

$0.01mol=\frac{\text{Mass of rust}}{159.7g/mol}\\\\\text{Mass of rust}=(0.01mol\times 159.7g/mol)=1.597g$

Hence, the mass of rust that can be removed is 1.597 grams

5 0

2 years ago

What is the pressure of the dry gas alone ?

gtnhenbr [62]

P O₂ = 736.2 torr

<h3>Further explanation</h3>

Given

P tot=760 torr

P H₂O = 23.8 torr

Required

P gas/O₂

Solution

Dalton's law of partial pressures stated that

the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases

Can be formulated:

P tot = P1 + P2 + P3 .... Pn

P tot = P H₂O + P O₂

760 torr = 23.8 torr + P O₂

P O₂ = 760 - 23.8

P O₂ = 736.2 torr

3 0

2 years ago