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3 years ago

Good chemistry question

1 answer:

5 0

Compared to the charge and mass of a proton an electron has......

A proton has approximately the same mass as..........

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The end point in a titration of a 58mL sample of aqueous HCl was reached by the addition of 25mL of 0.83MNaOH titrant. The react

Bess [88]

Answer:

0.36 M

Explanation:

Let's consider the following neutralization reaction.

HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)

25 mL of 0.83 M NaOH reacted. The moles of NaOH that reacted are:

0.025 L × 0.83 mol/L =0.021 mol

The molar ratio of NaOH to HCl is 1:1. The moles of HCl that reacted are 0.021 moles.

0.021 moles are contained in 58 mL of HCl. The molar concentration of HCl is:

M = 0.021 mol/0.058 L

M = 0.36 M

4 0

3 years ago

How many grams of potassium carbonate are needed to make 300ml of a 4.5M solution?

kenny6666 [7]

Answer:

186.3g

Explanation:

4.5moles of K₂CO₃ is in 1000ml

? moles of K₂CO₃ is in 300 ml

(4.5 × 300)/ 1000 = 1.35 moles of K₂CO₃

1 mole of K₂CO₃ = (39 × 2) + 12 + (16 × 3) = 78 + 12 + 48 = 138g

1.35 moles of K₂CO₃ = ?

= (1.35 × 138)/1 = 186.3g

4 0

2 years ago

How many grams of glucose, C6H12O6, in 2.47 mole?

statuscvo [17]

First, we need to find the atomic mass of $C_{6}H_{12}O_{6}$ .

According to the periodic table:
The atomic mass of Carbon = C = 12.01
The atomic mass of Hydrogen = H = 1.008
The atomic mass of Oxygen = O = 16

As there are 6 Carbons, 12 Hydrogens and 6 Oxygens, therefore:
The molar mass of   $C_{6}H_{12}O_{6}$ = 6 * 12.01 + 12 * 1.008 + 6 * 16

The molar mass of   $C_{6}H_{12}O_{6}$ = 180.156 grams/mole

Now that we have the molar mass of   $C_{6}H_{12}O_{6}$ , we can find the grams of glucose by using:

mass(of glucose in grams) = moles(of glucose given in moles) * molar mass(in grams/mole)

Therefore,
mass(of glucose in grams) = 2.47 * 180.156
mass(of glucose in grams = 444.99 grams

Ans: Mass of glucose in grams in 2.47 moles = 444.99 grams

-i

6 0

2 years ago

Read 2 more answers

What happens to the energy absorbed during an endothermic reaction

LuckyWell [14K]

Answer:

more energy is absorbed when the bonds in the reactants are broken

4 0

1 year ago

(c) O2 gas is transferred from a 3 L vessel containing oxygen at 4 atm to an evacuated 20 L vessel at a constant temperature of

Fudgin [204]

Answer:

After the transfer the pressure inside the 20 L vessel is 0.6 atm.

Explanation:

Considering O2 as an ideal gas, it is at an initial state (1) with V1 = 3L and P1 = 4 atm. And a final state (2) with V2 = 20L. The temperature remain constant at all the process, thus here applies the Boyle-Mariotte law. This law establishes that at a constant temperature an ideal gas the relationship between pressure and volume remain constant at all time:

$P x V = k$

Therefore, for this problem the step by step explanation is:

$P_{1} xV_{1} = P_{2} xV_{2}$

Clearing P2 and replacing

$P_{2}= \frac{P_{1} xV_{1}}{V_{2} } = \frac{4atmx3L}{20L} = 0.6atm$

7 0

3 years ago