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3 years ago

How many moles are present in 1.75 moles of dihydrogen monoxide, H2O?

Chemistry

1 answer:

KATRIN_1 [288]3 years ago

5 0

Answer:

31.5 grams

Explanation:

I'm guessing you meant how many grams are in 1.75 moles of H2O

You need a periodic table for this first you're going to find the atomic mass for Hydrogen (1.008) and oxygen (15.999)

since there are 2 Hydrogen in the problem you'll multiply 1.008 by 2 giving you 2.016

You'll then add your 1 Nitrogen to this to get 18.015: this number is the grams for 1 mole of H2O, you'll then multiply 18.015 by 1.75 to find the grams for that many moles (31.52625) this is how many grams are in 1.75 moles of H2O

Don't forget sig figs though so your answer will be 31.5

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What is the best description of the relationship between emerging scientific ideas and open-mindedness?

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Answer:

The main relationship between emerging scientific ideas and open-mindedness is that for many new ideas to be accepted a population has to have an open mind, otherwise the new ideas are rejected without thought.

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3 years ago

Define<br>Equivalent weight of a<br>Chemical substance

SSSSS [86.1K]

Equivalent weight, in chemistry, the quantity of a substance that exactly reacts with, or is equal to the combining value of, an arbitrarily fixed quantity of another substance in a particular reaction. ... The equivalent weight of an element is its gram atomic weight divided by its valence (combining power).

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2 years ago

write equations to show the chemical processes which occur when the first ionization and the second ionization energies of lithi

diamong [38]

Answer:

First ionization of lithium:

$\text{Li}\;(g)\to \text{Li}^{+} \; (g) + \text{e}^{-}$ .

Second ionization of lithium:

$\text{Li}^{+}\;(g) \to\text{Li}^{2+} \;(g) + \text{e}^{-}$ .

Explanation:

The ionization energy of an element is the energy required to remove the outermost electron from an atom or ion of the element in gaseous state. (Refer to your textbook for a more precise definition.) Some features of the equation:

Start with a gaseous atom (for the first ionization energy only) or a gaseous ion. Write the gaseous state symbol $(g)$ next to any atom or ion in the equation.
The product shall contain one gaseous ion and one electron. The charge on the ion shall be the same as the order of the ionization energy. For the second ionization energy, the ion shall carry a charge of +2.
Charge shall balance on the two sides of the equation.

First Ionization Energy of Li:

The products shall contain a gaseous ion with charge +1 $\text{Li}^{+}\;(g)$ as well as an electron $\text{e}^{-}$ .
Charge shall balance on the two sides. There's no net charge on the product side. Neither shall there be a charge on the reactant side. The only reactant shall be a lithium atom which is both gaseous and neutral: $\text{Li}\;(g)$ .

Hence the equation: $\text{Li}\;(g) \to \text{Li}^{+}\;(g) + \text{e}^{-}$ .

Second Ionization Energy of Li:

The product shall contain a gaseous ion with charge +2: $\text{Li}^{2+}\;(g)$ as well as an electron $\text{e}^{-}$ .
Charge shall balance on the two sides. What's the net charge on the product side? That shall also be the charge on the reactant side. What will be the reactant?

The equation for this process is $\text{Li}^{+} \; (g) \to \text{Li}^{2+}\;(g) + \text{e}^{-}$ .

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3 years ago

30. How many types of chemical reactions are there?

Nadusha1986 [10]

Answer:

B. Five

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3 years ago

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yaroslaw [1]

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1 year ago