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3 years ago

How is technology similar to printing words on a page?

2 answers:

6 0

Because your still writing whether its on an online document or writing on a piece of paper.Its the same thing

Hope this helped :))

lesantik [10]3 years ago

5 0

Because on both of them you are typing/writing something.

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Calculate the density of the four solutions. All of the solutions has the volume equal to 25 ml. Red solution has 25.0 g of mass

Scilla [17]

Answer:

B. Green solution density is 1.06 g/ml and blue solution density is 1.20 g/ml

Explanation:

Density is given as,

D = Mass / Volume

Red Solution,

D = 25 g / 25 mL

D = 1 g/mL

Green Solution,

D = 26.5 g / 25 mL

D = 1.06 g/mL

Yellow Solution,

D = 28.2 g / 25 mL

D = 1.128 g/mL

Blue Solution,

D = 30 g / 25 mL

D = 1.20 g/mL

3 0

3 years ago

____ KClO3-----> ____ KCl + ____O3

djyliett [7]

Answer:

explain what need to be done here pls? what do you need?

Explanation:

6 0

3 years ago

Read 2 more answers

Titanium and chlorine react to form titanium(IV) chloride, like this:

leva [86]

Answer:

the value of equilibrium constant for the reaction is 8.5 * 10⁷

Explanation:

Ti(s) + 2 Cl₂(g) ⇄ TiCl₄(l)

equilibrium constant Kc = $\frac{1}{[Cl_2]^2}$

Given that,

We are given:

Equilibrium amount of titanium = 2.93 g

Equilibrium amount of titanium tetrachloride = 2.02 g

Equilibrium amount of chlorine gas = 1.67 g

We calculate the No of mole = mass / molar mass

mass of chlorine gas = 1.67 g

Molar mass of chlorine gas = 71 g/mol

mole of chlorine = 1.67 / 71

= 7.0L

Concentration of chlorine is = no of mole / volume

= 0.024 / 7

= 3.43 * 10⁻³M

equilibrium constant Kc = $\frac{1}{[Cl_2]^2}$

= $\frac{1}{[3.43 * 10^-^3]^2}$

= 8.5 * 10⁷

4 0

3 years ago

Answer please!!!!!!!!!!!!!!!!!!!!!!!!✌✌✌

Nadya [2.5K]

Answer:

hxtististsy z7tzotz8tsx lhsitzrizrs ypzyztozkt udriztkzto

3 0

3 years ago

The reactant concentration in a second-order reaction was 0.560 m after 115 s and 3.30×10−2 m after 735 s . what is the rate con

Aloiza [94]

Use the formula for second order reaction:

$\frac{1}{C} = \frac{1}{C_0} + kt$

C = concentration at time t
C0 = initial conc.
k = rate constant
t = time

1st equation : $\frac{1}{0.56} = \frac{1}{C_0} + 115k$

2nd Equation: $\frac{1}{0.033} = \frac{1}{C_0} + 735k$

Find $\frac{1}{C_0}$ from 1st equation and put it in 2nd equation:

$\frac{1}{0.033} = \frac{1}{0.56} - 115k + 735k$

$\frac{1}{0.033} - \frac{1}{0.56} = 620k$

k = 0.046

3 0

3 years ago