All categories

2 years ago

2. What was the primary goal of the Apollo program?

Chemistry

2 answers:

Ivenika [448]2 years ago

7 0

The right answer is bbbbb

babunello [35]2 years ago

3 0

Answer:

Explanation:

to conduct scientific exploration of the moon

You might be interested in

Vanillin, C8H8O3, is the active ingredient in vanilla flavoring. It contains a six-membered aromatic ring with an aldehyde group

dlinn [17]

Answer:

The answer is in the picture attached

Explanation:

A six-membered aromatic ring is one of the most common structures in natural compounds.

The aldehyde group in position one consist in one carbon double-bonded to oxygen and bonded to hydrogen.

The alkoxy group in position three consist in a oxygen bonded to an alkyl group (The simplest alkyl group is methyl -CH₃-).

There is, in position four, an hydroxyl group -OH. bonded to this six-membered aromatic ring.

I hope it helps!

3 0

3 years ago

B The allusions recall specific locations and horrors of the Vietnam conflict.How many moles of H2O are produced when 12 moles o

ziro4ka [17]

<u>Answer:</u> 18 moles of $H_2O$ will be produced.

<u>Explanation:</u>

We are given:

Moles of ammonia = 12 moles

The given chemical equation follows:

$4NH_3+5O_2\rightarrow 4NO+6H_2O$

By the stoichiometry of the reaction:

4 moles of ammonia produces 6 moles of water

So, 12 moles of ammonia will produce = $\frac{6}{4}\times 12=18mol$ of water

Hence, 18 moles of $H_2O$ will be produced.

7 0

2 years ago

Use the periodic table to help you.

BARSIC [14]

The answer would be Sb
Because N P and O are all non metals whereas Sb is a metal

7 0

3 years ago

Read 2 more answers

For the equilibrium

sleet_krkn [62]

Answer:

$\large \boxed{\text{0.091 atm }}$

Explanation:

The balanced equation is

I₂(g) + Br₂(g) ⇌ 2IBr(g)

Data:

Kc = 8.50 × 10⁻³

n(IBr) = 0.0600 mol

V = 1.0 L

1. Calculate [IBr]

$\text{[IBr]} = \dfrac{\text{0.0600 mol}}{\text{1.0 L}} = \text{0.0600 mol/L}$

2. Set up an ICE table.

$\begin{array}{ccccccc}\rm \text{I}_{2}& + & \text{Br}_{2} & \, \rightleftharpoons \, & \text{2IBr} & & \\0 & & 0 & &0.0600 & & \\+x & & +x & &- 2x & & \\x & & x & & 0.0600 - 2x & & \\\end{array}$

3. Calculate [I₂]

$\begin{array}{rcl}K_{\text{c}}&=&\dfrac{\text{[IBr]}^{2}} {\text{[I$_{2}$][Br]$_{2}$}}\\\\8.50 \times 10^{-2}&=&{\dfrac{(0.0600 - 2x)^{2}}{x^{2}}}& &\\\\0.2915x & = &{\dfrac{0.0600 - 2x}{x}}& &\\\\0.2915x & = &0.0600 - 2x\\\\2.2915x & = & 0.0600\\x & = & \textbf{0.026 18 mol/L}\\\end{array}\\$

4. Convert the temperature to kelvins

T = (150 + 273.15) K = 423.15 K

5. Calculate p(I₂)

$\begin{array}{rcl}\\pV & = & nRT\\p & = & cRT\\p & = & \text{0.026 18 mol} \cdot \text{L}^{-1}\times \text{0.082 06 L} \cdot \text{atm} \cdot \text{K}^{-1} \text{mol}^{-1} \times \text{423.15 K}\\& = & \textbf{0.91 atm}\\\end{array}\\\text{The partial pressure of iodine is $\large \boxed{\textbf{0.91 atm}}$}$

6 0

3 years ago

Câu 47: Cách pha chế dung dịch từ hoá chất tinh khiết, phát biểu sai:

VashaNatasha [74]

Answer:

Explanation:

6 0

2 years ago