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3 years ago

Can you substitute evaporated milk for condensed milk

1 answer:

3 0

Yes because condensed milk and evaporated milk are similar to one another. However, there won’t be the same sweet flavor but the texture is the same.

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When 125 grams of FeO react with 25.0 grams of Al, how many grams of Fe can be produced? FeO + Al → Fe + Al2O3 25.9 g Fe 38.7 g

Serga [27]

Answer: The mass of iron produced will be 77.6 grams

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For FeO:

Given mass of FeO = 125 g

Molar mass of FeO = 71.8 g/mol

Putting values in equation 1, we get:

$\text{Moles of FeO}=\frac{125g}{71.8g/mol}=1.74mol$

For aluminium:

Given mass of aluminium = 25.0 g

Molar mass of aluminium = 27 g/mol

Putting values in equation 1, we get:

$\text{Moles of aluminium}=\frac{25.0g}{27g/mol}=0.93mol$

The given chemical reaction follows:

$3FeO+2Al\rightarrow 3Fe+Al_2O_3$

By Stoichiometry of the reaction:

2 moles of aluminium metal reacts with 3 mole of FeO

So, 0.93 moles of aluminium metal will react with = $\frac{3}{2}\times 0.93=1.395mol$ of FeO

As, given amount of FeO is more than the required amount. So, it is considered as an excess reagent.

Thus, aluminium metal is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of aluminium metal produces 3 mole of iron metal

So, 0.93 moles of aluminium metal will produce = $\frac{3}{2}\times 0.93=1.395moles$ of iron metal

Now, calculating the mass of iron metal from equation 1, we get:

Molar mass of iron = 55.85 g/mol

Moles of iron = 1.395 moles

Putting values in equation 1, we get:

$1.395mol=\frac{\text{Mass of iron}}{55.85g/mol}\\\\\text{Mass of iron}=(1.395mol\times 55.85g/mol)=77.6g$

Hence, the mass of iron produced will be 77.6 grams

4 0

3 years ago

Write a balanced equation formed when the following elements react with oxygen:a)Zinc

Ainat [17]

Explanation:

a) when zinc burnt in oxygen.

2Zn + O2 -----∆-----> 2ZnO(black residue)

b) when carbon burnt in oxygen.

C+O2----∆---> CO2.

c) when sulphur burnt in oxygen.

S+O2-----∆-----> SO2.

d) when Calcium burnt in oxygen.

2Ca+O2-----∆-----> 2CaO(black residue)

e) when Magnesium burnt in oxygen.

2Mg+O2-----∆----> 2MgO.

f) when sodium burnt in oxygen.

4Na+O2----∆-----> 2Na2O.

hope all these reactions help you.

4 0

3 years ago

What mass of zinc is needed to react with 23.1g of phosphoric acid according to the following equation?

Hunter-Best [27]

23.01 g of zinc (Zn)

Explanation:

We have the following chemical reaction:

3 Zn + 2 H₃PO₄ = 3 H₂ + Zn₃(PO₄)₂

number of moles = mass / molar weight

number of moles of phosphoric acid = 23.1 / 98 = 0.236 moles

Taking in account the chemical reaction, we devise the following reasoning:

if 2 moles of H₃PO₄ are reacting with 3 moles of Zn

then 0.236 moles of H₃PO₄ are reacting with X moles of Zn

X = (0.236 × 3) / 2 = 0.354 moles of Zn

mass = number of moles × molar weight

mass of Zn = 0.354 × 65 = 23.01 g

Learn more about:

number of moles

brainly.com/question/13911775

#learnwithBrainly

5 0

3 years ago

Which type of scientist would observe the spread of a species of red fire ants

diamong [38]

It would be a biologist

7 0

3 years ago

What volume does 14 mol of gas occupy at STP? Round to the nearest hundredth.

Anna007 [38]

Answer:

The volume is 310 L

Explanation:

We use the ideal gas formula, with the constant R = 0.082 l atm / K mol. The STP conditions are 1 atm pressure and 273 K temperature. Solve for the formula, V (volume):

PV= nRT ---> V= (nRT)/P

V=( 14 mol x 0,082 l atm /K mol x 273 K)/ 1 atm

V= 313,404 L

4 0

3 years ago